Locate fluorine (F) on the partial periodic table provided in Figure 2.2. Predict its relative electronegativity compared to hydrogen, sodium, and oxygen. State the number and type of bond(s) you expect it would form if it reacted with sodium (Na).

Electronegativity is a measure of an atom's ability to attract and hold onto electrons when forming chemical bonds. It is a key factor in determining how atoms interact with each other. In the periodic table, electronegativity generally increases from left to right across a period and decreases from top to bottom within a group. Fluorine, being in the top right corner, is the most electronegative element, which means it has a strong tendency to attract electrons compared to hydrogen, sodium, and oxygen.

Ionic bonding occurs when one atom donates an electron to another, resulting in the formation of charged ions. This type of bond typically forms between metals and nonmetals, where the metal loses electrons and the nonmetal gains them. In the case of sodium (Na) and fluorine (F), sodium will lose one electron to become Na+, while fluorine will gain that electron to become F-. This transfer of electrons leads to the formation of an ionic bond between the two elements.

Periodic trends refer to the predictable patterns observed in the properties of elements as you move across or down the periodic table. These trends include variations in atomic size, ionization energy, and electronegativity. Understanding these trends helps predict how different elements will interact chemically. For example, as you move from sodium to fluorine, the increasing electronegativity of fluorine indicates it will form a stronger bond with sodium than sodium would with hydrogen or oxygen.